Answer:
65 L is the volume of CO required
Explanation:
This is the reaction:
2CO (g) + O₂ (g) → 2CO₂ (g)
We must work with density to solve this problem
Density = Mass / volume
Let's determine the moles of O₂
1.43 g/mL = mass / 32500 mL
Notice, that we had to convert the volume from L, to mL, because the units of density.
Mass of O₂ → 1.43 g/mL . 32500 mL = 46475 g
Let's convert the mass to moles (mass / molar mas)
46475 g / 32 g/mol = 1452.3 moles
So ratio is 1:2
1 mol of oxygen needs 2 moles of CO, to react
Then, 1452.3 moles of O₂ would need the double of CO to react
1452.3 moles . 2 = 2904.6 moles of CO
This moles are contained in (mol . molar mass) =
2904.6 mol . 28 g/mol =81328.8 g
Density of CO = Mass of CO/ Volume of CO
1.25 g/mL = 81328.8 g / Volume of CO
81328.8 g / 1.25 g/mL = 65063 mL
If we convert to L
65063 mL = 65.0 L
